Calculate the pH of a 1.0 × 10-* M solution of HBr. Be sure your answer has the correct number of significant figures.

1 answer

To calculate the pH of a solution of HBr, which is a strong acid that ionizes completely in solution, you can use the formula:

\[ \text{pH} = -\log[\text{H}^+] \]

In this case, since the concentration of HBr is \(1.0 \times 10^{-1}\) M, the concentration of hydrogen ions \([\text{H}^+]\) will also be \(1.0 \times 10^{-1}\) M.

Now, we can calculate the pH:

\[ \text{pH} = -\log(1.0 \times 10^{-1}) \]

Calculating the logarithm:

\[ \log(1.0 \times 10^{-1}) = -1 \]

So,

\[ \text{pH} = -(-1) = 1.0 \]

Thus, the pH of the \(1.0 \times 10^{-1}\) M solution of HBr is:

\[ \text{pH} = 1.0 \]

Since the original concentration was given to two significant figures, we can express the pH with the same significant figures:

\[ \text{pH} = 1.0 \]

So, the answer is 1.0.